IX-CHEMISTRY
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IX-CHEMISTRY
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IX-CHEMISTRY
PERIODIC CLASSIFICATION - 2
SYNOPSIS - 3
________________________________________________________________________________
MODERN PERIODIC TABLE
Introduction: In 1913 Moseley found that frequency of X-ray emitted by different
elements is directly proportional to the atomic number.
υ = a  z - b  where,
υ = frequency of emitted x-ray
a, b are constant.
z = atomic number.
These studies shows that properties of elements depends upon the atomic number but
not atomic mass.
So atomic number is the basis of classification of the element. Moseley gave modern
periodic law which stated as “The physical and chemical properties of the elements are
periodic functions of their atomic number”
In this table, elements have been arranged in order of increasing atomic number. This
table consists of groups and periods which are discussed as below:
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IX-CHEMISTRY
Groups:
i)
The vertical columns in the periodic table are called groups.
ii) There are 18 groups designated as 1 to 18. (or)
I(A)-VII(A), I(B)-VII(B), VIII & O Group.
(In VIII group three sub groups are present)
iii) All the elements in a group have same number of electrons in the outermost
shell.(orbit).
iv) The elements of each group have similar chemical properties due to same valence
electrons.
The periodic table groups are as follows:
NEW IUPAC
OLD IUPAC
CAS
NUMBERING
(EUROPEAN) (AMERICAN)
NAME
Group 1
IA
IA
The alkali metals
Group 2
IIA
IIA
The alkaline earth metals.
Group 3
IIIA
IIIB
The scandium family
Group 4
IVA
IVB
The Titanium family
Group 5
VA
VB
The Vanadium family
Group 6
VIA
VIB
The Chromium family
Group 7
VIIA
VIIB
The Manganese family
Group 8
VIII
VIIIB
The Iron family
Group 9
VIII
VIIIB
The cobalt family
Group 10
VIII
VIIIB
The nickel family
Group 11
IB
IB
The coinage metals or copper family
Group 12
IIB
IIB
The zinc family
Group 13
IIIB
IIIA
The boron group or boron family
Group 14
IVB
IVA
The carbon group or carbon family
Group 15
VB
VA
The pnicogens or nitrogen family
Group 16
VIB
VIA
The chalcogens or oxygen family
Group 17
VIIB
VIIA
The halogens or fluorine family
Group 18
Group 0
VIIIA
The noble gases or helium family (or)
Inert gases (or) rare gases.
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Periods:
i)
The horizontal rows are called Periods.
ii) Totally seven periods are present in the modern periodic table.
iii) All period’s starts from alkali metals and ends with inert gases.
1st period:
(a) It starts with H(1) and ends with He(2).
(b) It contains 2 elements.
(c) It is called very short period.
(d) In this 1s energy level is present.
2nd period: (a) It starts with Li (3) and ends with Ne(10).
(b) It contains 8 elements.
(c) It is called short period.
(d) In this 2s & 2p energy levels are present.
3rd period: (a) It starts with Na (11) and ends with Ar (18).
(b) It contains 8 elements.
(c) It is called short period.
(d) In this 3s & 3p energy levels are present.
4th period:
(a) It starts with K (19) and ends with Kr (36).
(b) It contains 18 elements.
(c) It is called long period.
(d) In this 4s, 4p and 3d energy levels are present.
5th period:
(a) It starts with Rb (37) and ends with Xe (54).
(b) It contains 18 elements.
(c) It is called long period.
(d) In this 5s, 5p & 4d energy levels are present.
6th period:
(a) It starts with Cs (55) and ends with Rn (86).
(b) It contains 32 elements.
(c) It is called very longest period.
(d) In this 6s, 6p, 5d & 4f energy levels are present.
7th period:
(a) It starts with Fr (87).
(b) It is an incomplete period.
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IX-CHEMISTRY
1.
2.
Properties
Periods
Groups
Valence
On moving from left to right
All the elements of a group of
electrons
in a period, the number of
the periodic table have the
valance electrons in elements
same number of valance
increases from 1 to 8.
electrons
On moving from left to right
The valency of a metal is
in each short period, The
equal to its group number in
valency of elements increases
the periodic table. The
from 1 to 4 and then
valency of non-metal is equal
decrease to 0.
to 8 minutes group number in
Valency
the periodic table.
3.
Size of atoms
On moving from left to right
Ongoing down in a group of
in a period of the periodic
the periodic table, the size of
table the size of atoms
atoms increases.
decreases.
4.
5.
Metallic
On moving from left to right
Ongoing down in a group of
character
in a period, the metallic
the periodic table, the
character of elements
metallic character of elements
decreases but the non-
increases but non-metallic
metallic character increases.
character decreases.
Chemical
On moving from left to right
The chemical reactivity of
reactivity
in a period, the chemical
metals increases on going
reactivity of elements first
down in a group of the
decreases and then
periodic table. The chemical
increases.
reactivity of non-metal
decreases on going down in a
group of the periodic table.
6.
Nature of oxides
On moving from left to right
Ongoing down in a group of
in a period, the basic nature
the periodic table, there is no
of oxides decreases and the
change in the nature of oxides
acidic nature of oxides
of elements.
increases
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7.
Ionization
Ionization energy generally
Ionization energy decreases
potential
increases from left to right
from top to bottom in a group
along a periodic because the
because of the increase in a
atomic size of the elements
atomic radius which is due to
gradually decreases due to
the increase in the number of
the increases in the atomic
shells.
number.
8.
9.
Electron affinity
Electron affinity values
Electron affinity gradually
generally increases on
decreases from top to bottom
moving from left to right
in a group. This is due to the
along a period due to the
steady increase in the atomic
decrease in the atomic size
radius and the decrease in
and the increase in its
the effective nuclear charge of
effective nuclear charge.
the elements.
Electro-
Electronegativity increases
Electronegativity decreases
negativity
on moving along a period
from top to bottom in a group
from left to right. This is due
due to an increase in the
to the increase in nuclear
atomic size, as a result of
charge and decrease in
which the shared electron
atomic size, as a result of
pair is attracted less towards
which shared electron pair
itself
can be attracted more
towards itself.
10. Oxidizing/
Due to the increase in
Due to the decrease in
reducing
electron affinity from left to
ionization potential as well as
capacity
right of a period, the
electron affinity from top to
oxidizing capacity of the
bottom of a group, oxidizing
elements increases and the
capacity of the element
reducing capacity decreases
decreases whereas it’s
from left to right along a
reducing capacity increase on
period.
moving down a group.
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IX-CHEMISTRY
Merits of the long form of periodic table:
i)
The classification is based on the atomic number of elements, which is more
fundamental than the atomic weight.
ii) In this periodic table, the position of an element is related to the electronic
configuration of the atom. Elements belonging to the same group possess same
number of electrons in their valence shells and show similar chemical characteristics.
Element
Atomic
No. of
Electronic
No. of electrons
number
shells
configuration
in valence shell
Alkali
Li
3
2
2, 1
1
metals
Na
11
3
2, 8, 1
1
K
19
4
2, 8, 8, 1
1
Rb
37
5
2, 8, 18, 8,1
1
Cs
55
6
2, 8, 18, 18, 8,1
1
Fr
87
7
2, 8, 18, 32, 18, 8,1
1
F
9
2
2, 7
7
Cl
17
3
2, 8, 7
7
Br
35
4
2, 8, 18, 7
7
I
53
5
2, 8, 18, 18, 7
7
At
85
6
2,8,18,32,18,7
7
Halogens
iii) Variation of chemical properties along a period is correlated with gradual filling of
electrons in a particular shell in the period.
iv) In this table, inert gases are placed at the end of each period which is very logical
because valence shells have octet configuration. So, their inertness can also be
explained in terms of the electronic configuration.
v) Due to the separation of the two subgroups, dissimilar elements (e.g. alkali and
coinage metals) do not fall together.
vi) Different types of elements like
i) active metals, ii) transition metals, iii) non-metals and metalloids
iv) noble gases and inner transition elements (lanthanides and actinides) have their
separate locations in this periodic table.
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IX-CHEMISTRY
Defects of the long-form of the periodic table:
i)
Even after the compilation of the modern periodic table, the position of hydrogen
remained controversial. This is because hydrogen with one electron in its valence
shell shows similarities with both alkali metals and halogens. Therefore, placing
hydrogen in IA group is not completely justifiable.
ii) The elements lanthanides and actinides could not be placed in the main body of the
modern periodic table.
iii) This periodic table does not reflect the exact distribution of electrons of some of the
transition and inner-transition elements.
Advantages of long form of periodic table:i)
The position of the elements is linked with their electronic configuration.
ii) Position of isotopes of an element is justified since they have same atomic number.
iii) Similar properties of element in a group is also justified due to same valence
electrons.
iv) Each group is an independent group and idea of sub-group discarded.
IUPAC nomenclature of elements with Z >100 (super heavy elements)
Super heavy elements are trans-Fermium elements, i.e., super heavy elements are those
which are placed after Fermium (Fm) (z = 100) in the long form of periodic table. In other
words these are the elements whose atomic number is greater than 100. For IUPAC
nomenclature of these elements the following rules have been proposed.
i)
Roots: The names have three roots which indicate the three digits of the atomic
number of the elements. In the last root–ium is added. The roots and symbols for the
digit are given below:
Digit
Root
Symbol
0
1
2
3
4
5
6
7
8
9
Nil Un Bi Tri Quad Pent Hex Sept Oct Enn
n
u
b
t
q
p
h
s
o
e
ii) Symbol: The symbol for the element has three letters derived from the roots.
iii) Name: The name of the element starts with a small letter but the symbol of the
element starts with a capital letter. The names are written as a complete word. The
above rules are clear from the following examples. In the IUPAC name column, a
hyphen (-) has been put between each part of the names to make them more
understandable. Present names and symbols of the elements with atomic number
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101 to 120 have also been given. Present names of other elements have not been
fixed as yet.
Atomic number
IUPAC name
Symbol
Present name
Symbol
101
Unnilunium
Unu
Mendelevium
Md
102
Unnilbium
Unb
Nobelium
No
103
Unniltrium
Unt
Lawrencium
Lr
104
Unnilquadium
Unq
Rutherfordium
Rf
105
Unnilpentium
Unp
Dubnium
Db
106
Unnilhexium
Unh
Seaborgium
Sg
107
UnnilSeptium
Uns
Bohrium
Bh
108
Unniloctium
Uno
Hassium
Hs
109
Unnilennium
Une
Meitherium
Mt
110
Ununnilium
Uun
Dermstadtium
Ds
111
Unununium
Uuu
Rontgenium
Rg
112
Ununbium
Uub
a
a
113
Ununtrium
Uut
a
-
114
Ununquadium
Uuq
a
a
115
Ununpentium
Uup
a
-
116
Ununhexium
Unh
a
a
117
Ununseptium
Uus
b
-
118
Ununoctium
Uuo
a
-
119
Ununennium
Uue
a
-
120
Unbinilium
Ubn
b
-
1. Define Moseley’s periodic law?
Solution: In 1913 Moseley found that frequency of X-ray emitted by different elements is
directly proportional to the atomic number.
v = a ( z - b) where,
v = frequency of emitted x-ray
a,b are constant
z = atomic number.
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IX-CHEMISTRY
2. Write a short notes on 1st period?
Solution:
1st period:
(a) It starts with H(1) and ends with He(2).
(b) It contains 2 elements.
(c) It is called very short period.
(d) In this 1s energy level is present
The modern periodic law proposed by Moseley. He found the relation between atomic
numbers (Z) and the frequencies (ν) of X-rays produced when the atoms of different
elements are bombarded with cathode rays. The relation between the square root of
frequency
   of highest energy emission line called Kα line, with the atomic number, Z
was found to be linear.
The mathematical relation can be presented as:
  a  Z  b
Where a & b are constants, characteristic of elements.
Later on it was clearly established that an element can be characterized by its atomic
number, Z and not by the atomic weight. It was also found that there is a relation between
electronic configuration and properties of elements. The number of electrons in an atom
and its electronic configuration are in turn are related to the atomic number.
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IX-CHEMISTRY
Merits of the long form of periodic table:
i)
The classification is based on the atomic number of elements, which is more
fundamental than the atomic weight.
ii) In this periodic table, the position of an element is related to the electronic
configuration of the atom. Elements belonging to the same group possess same
number of electrons in their valence shells and show similar chemical characteristics.
Element
Atomic
No. of
Electronic
No. of electrons
number
shells
configuration
in valence shell
Alkali
Li
3
2
2, 1
1
metals
Na
11
3
2, 8, 1
1
K
19
4
2, 8, 8, 1
1
Rb
37
5
2, 8, 18, 8,1
1
Cs
55
6
2, 8, 18, 18, 8,1
1
Fr
87
7
2, 8, 18, 32, 18, 8,1
1
F
9
2
2, 7
7
Cl
17
3
2, 8, 7
7
Br
35
4
2, 8, 18, 7
7
I
53
5
2, 8, 18, 18, 7
7
At
85
6
2,8,18,32,18,7
7
Halogens
Advantages of long form of periodic table:
i)
The position of the elements is linked with their electronic configuration.
ii) Position of isotopes of an element is justified since they have same atomic number.
iii) Similar properties of element in a group is also justified due to same valence
electrons.
iv) Each group is an independent group and idea of sub-group discarded.
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Atomic number
Iupac name
Symbol
Present name
Symbol
101
Unnilunium
Unu
Mendelevium
Md
102
Unnilbium
Unb
Nobelium
No
103
Unniltrium
Unt
Lawrencium
Lr
104
Unnilquadium
Unq
Rutherfordium Rf
105
Unnilpentium
Unp
Dubnium
Db
106
Unnilhexium
Unh
Seaborgium
Sg
107
UnnilSeptium
Uns
Bohrium
Bh
108
Unniloctium
Uno
Hassium
Hs
109
Unnilennium
Une
Meitherium
Mt
110
Ununnilium
Uun
Dermstadtium
Ds
111
Unununium
Uuu
Rontgenium
Rg
112
Ununbium
Uub
a
a
113
Ununtrium
Uut
a
-
114
Ununquadium
Uuq
a
a
115
Ununpentium
Uup
a
-
116
Ununhexium
Unh
a
a
117
Ununseptium
Uus
b
-
118
Ununoctium
Uuo
a
-
119
Ununennium
Uue
a
-
120
Unbinilium
Ubn
b
-
1. Mention the advantages of long-form of periodic law?
2. Write a short notes on super heavy metals?
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IX-CHEMISTRY
MODERN PERIODIC TABLE
EXERCISE - 3
LEVEL - I
SINGLE CORRECT CHOICE TYPE:
1. The number of periods present in the long form of the periodic table.
A) 6
B) 7
C) 8
D) 18
[
]
2. The longest and shortest periods are.
[
]
A) 1 & 6
B) 2 & 6
C) 6 &1
D) 1 & 7
3. What would be the IUPAC name and symbol for the element with atomic number
120?
[
A) Unnilbium (Unb)
B) Unbinilium (Ubn)
C) Unnilunium (Unu)
]
D) Unniltrium (Unt)
4. Write the respective names given by IUPAC to the elements named Unununium
Ununnilium, unnilennium?
[
]
A) Meitnerium, Hassium, Bohrium
B) Darmstadtium, Meitnerium, Hassium
C) Rontgenium, Darmstadtium, Meitnerium
D) None
5. The atomic number of the element named after the scientist who introduced the
concepts of orbits or main energy levels:
[
]
A) 107
B) 108
C) 109
D)
110
6. Which pair of elements of atomic number given below will have similar chemical
properties?
[
A) 13, 22
B) 19, 11
C) 4, 24
]
D) 2, 4
REASONING TYPE:
7. Statement I: The group 18 consists of elements which are in gaseous state under
ordinary condition.
Statement II: All the elements of group 18 called as inert gases.
[
A) Both Statements are true.
B) Both Statements are false.
C) Statement I is true. Statement II is false.
D) Statement I is false. Statement II is true.
]
MULTI CORRECT CHOICE TYPE:
8. Which of the following elements belongs to 2nd period.
A) Li
B) Be
C) B
]
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[
D) Na
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IX-CHEMISTRY
INTEGER TYPE:
9. The number of elements present in 4th period of modern periodic table is ________.
LEVEL - II
SINGLE CORRECT CHOICE TYPE:
10. An element with atomic number 20 will be placed in which period of the periodic
table?
[
A) 4
B) 3
C) 2
D) 1
11. Element with atomic number 15 and mass number 31 is present in:
A) Group 5 and period 4
C) Group 15 and period 3
[
]
]
B) Group 6 and period 3
D) Group 15 and period 4
12. Which of the following pair of elements are from the same group of the periodic
table.
[
A) Mg, Cs
B) Mg, Sr
C) Mg, Cl
D) Na, Cl
]
REASONING TYPE:
13. Statement I: An element with atomic number 50 must exhibit properties similar to
the properties of lead.
[
]
Statement II: The elements with atomic numbers 10,18,36,54 and 86 are called inert
gases.
A) Both Statements are true.
B) Both Statements are false.
C) Statement I is true. Statement II is false.
D) Statement I is false. Statement II is true.
MULTI CORRECT CHOICE TYPE:
14. The atomic numbers of few elements are given below: Which of them can be
considered as trans-fermium elements?
[
]
A) 101
B) 105
C) 93
D) 96
LEVEL - III
SINGLE CORRECT CHOICE TYPE:
15. The 100th element is named in honour of:
A) Einstein
B) Bohr
[
C) Fermi
]
D) Maolame curie
16. The 3d-transition series contains elements having atomic numbers ranging from:[ ]
A) 22 to 31
B) 21 to 31
C) 21 to 30
D) 39 to 48
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LINKED COMPREHENSION PASSAGE:
The salient features of periods are: i) Seven horizontal rows of the periodic table are
known as periods. ii) Each period begins with the outermost electron entering into a
new principal quantum number and completes after the outer-most shell’s p-subshell
is complete. iii) The number of period denotes the number of outermost shell of that
element. iv) The first element of each period (except 1 period) is an alkali metal and
the last element is an inert gas.
17. The atomic number of an element ‘X’ is 34. Then it is present in ___________ period
and __________ in group.
A) 4th period and IVA group.
B) 4th Period and VIA group.
C) 4th period and VIIA group.
D) 5th period and VIA group.
18. The position of element with Z = 24 in the periodic table as:
A) VA group and 4th period.
B) VIB group and 4th period.
C) IVA group and 3rd period.
D) IIIB group and 3rd period.
[
]
[
]
19. In which of the following period a maximum number of 32 elements are present?[
A) 4
B) 6
MATRIX MATCH TYPE:
20.
Column - I
C) 3
]
D) 7
Column - II
a) Pnicogens
p) Fluorine family
b) Chalcogens
q) Nitrogen family
c) Halogens
r) Helium family
d) Aerogens
s) Oxygen family
t) Carbon family
MODERN PERIODIC TABLE, SUPER HEAVY ELEMENTS
Q1
Q2
Q3
Q4
Q5
Q6
Q7
B
C
B
C
A
B
A
Q11
Q12
Q13
Q14
Q15
Q16
Q17
C
B
A
A,B
C
C
B
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Q8
A,B,C
Q18
B
Q9
18
Q19
B
EXERCISE - 3
Q10
A
Q20
a-q; b-s; c-p; d-r
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PERIODIC CLASSIFICATION - 2
MODERN PERIODIC TABLE
1. Advantages of long form of periodic table:
v) The position of the elements is linked with their electronic configuration.
vi) Position of isotopes of an element is justified since they have same atomic number.
vii) Similar properties of element in a group is also justified due to same valence
electrons.
Each group is an independent group and idea of sub-group discarded.
2. Super heavy elements are trans-Fermium elements, i.e., super heavy elements are
those which are placed after Fermium (Fm) (z = 100) in the long form of periodic table. In
other words these are the elements whose atomic number is greater than 100. For
IUPAC nomenclature of these elements the following rules have been proposed.
i)
Roots: The names have three roots which indicate the three digits of the atomic
number of the elements. In the last root–ium is added. The roots and symbols for the
digit are given below:
Digit
Root
Symbol
0
1
2
3
4
5
6
7
8
9
Nil Un Bi Tri Quad Pent Hex Sept Oct Enn
n
u
b
t
q
p
h
s
o
e
ii) Symbol: The symbol for the element has three letters derived from the roots.
iii) Name: The name of the element starts with a small letter but the symbol of the
element starts with a capital letter. The names are written as a complete word. The
above rules are clear from the following examples. In the IUPAC name column, a
hyphen (-) has been put between each part of the names to make them more
understandable. Present names and symbols of the elements with atomic number
101 to 120 have also been given. Present names of other elements have not been
fixed as yet.
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IX-CHEMISTRY
EXERCISE - 3
1. Totally 7 periods are present in modern periodic table. Option B is correct.
2. In modern periodic table longest period is 6 and short period is 1. Option C is
correct.
3. According to IUPAC name and symbol for the element with atomic number 120 is
Unbinilium (Ubn). Option B is correct.
4. Unununium (Uuu) – Rontgenium with atomic number – 111
Ununnilium – (Uun) Darmstadtium with atomic number – 110
Unnilennium – (Une) – Meitnerium with atomic number – 109. Option C is correct.
5. The concept of orbit (shell) or main energy levels was given by Neil’s Bohr atomic
number – 107 – named with his name as Bohrium (Unnil septium). Option A is correct.
6. Atomic number 19 = K
Atomic number 11 = Na
Na and K are first group elements they will show the similar chemical properties.
Option B is correct
7. Inert gases (or) Nobel gases have stable electronic configuration and they are gases at
room temperature. Option A is correct.
8. Li to Ne (8) elements belongs to 2nd period. Options A,B and C are correct.
9. The number of elements present in 4th period of modern periodic table is 18. Answer
is 18
10. An element with atomic number 20 will be placed in 4th period elements are belongs
to from atomic number (18 - 36). Option A is correct.
11. Element is phosphorous, arranged in 3rd period and 15th group of a periodic table.
Option C is correct.
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12. Mg, Sr belongs to 2nd group elements, called as alkaline earth metals. Option B is
correct.
13. An element with atomic number 50(tin) must exhibit properties similar to the
properties of lead because both are in same group. The elements with atomic
numbers 10,18,36,54 and 86 are called inert gases. Option A is correct.
14. The elements which are placed after fermium (atomic number 100) are called transfermium elements. 101 – Mendelevium (Md), 105 – Dubnium (Db), are belongs to transfermium elements. Options A and B are correct.
15. 100th element is called Fermium (Fm) named in honour of Fermi. Option C is
correct
16. The 3d-transition series contains elements having atomic numbers ranging from
21 to 30. i.e., Scandium – 21 to Zinc – 30. Option C is correct


17. Atomic number 34 is selenium 3d10 4s 2 4p 4 it is 4th period and VIA group.
Option B is correct


18. The element with atomic number 24 is chromium 3d 5 4s1 it is 4th period and
VIB group element. Option B is correct
19. Sixth period has 32 elements  Cs 55 to Rn 86  . Option B is correct
20. a-q; b-s; c-p; d-r
a) Pnicogens - Nitrogen family
b) Chalcogens - Oxygen family
c) Halogens - Fluorine family
d) Aerogens - Helium family
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